College Preparatory Chemistry is a practical approach to the study of chemistry intended to improve students’ chemical literacy and ability to apply new concepts to problem solving situations. The goals of this course are for each student to have a positive science experience in an educationally challenging program and to insure “real world” and college science readiness. Feel free to contact me at any time with questions or concerns. Help is always accessible with appropriate communication.
Course Description
Students will explore the mechanisms of matter and chemical reactions through quantitative and qualitative analysis, while developing problem-solving skills, and learning accurate laboratory techniques. The course stresses an understanding of the basic theoretical concepts of chemistry with a strong emphasis on measurement and calculation. Topics include the atomic and molecular structure, periodicity, chemical bonding, the mole concept, chemical equations and reactions, stoichiometry, gas laws, acid/base reactions, and thermochemistry. Testing and assessment is built on a series of levels from basic knowledge to application and higher order thinking, and several laboratory activities per unit will be used to enhance the understanding of each chemical concept.
Required Materials
Text Book: Modern Chemistry, Holt, Rinehart and Winston
Thread-bound Composition Journal [For notes and labs]
How to Succeed in this Course:
(1) Attend EVERY class, come prepared and pay attention
(2) Work hard (there are no short-cuts in science)
(3) Think (an often underrated and underemployed skill)
Essential Learning Outcomes
Students will master the following standards through in-class lecture, homework, and lab work. Units are divided into related topics, where order and pace may vary according to student response to the material.
After completing CP Chemistry students will be able to:
A) attribute a state of matter to its molecular arrangement and freedom of motion
B) classify a substance as an element, compound, or mixture
C) analyze and compare physical and chemical properties of matter
D) describe the composition of matter in terms of atoms and subatomic particles
E) interpret the structure of the Periodic Table and use it to obtain information
F) recognize how the configuration of electrons governs the chemical properties of an element
G) explain how chemical bonding occurs and compare types of bonds
H) illustrate how molecules are consistently arranged in geometric patterns
I) describe how substances chemically react to form new substances with different properties
J) apply the mole concept to the meaning and uses of chemical equations
K) use stoichiometry to quantify relationships between products and reactants
L) describe and apply principles that effect the rate of chemical reactions
M) exemplify principles of ideal gas behavior
N) analyze aqueous solutions in terms of concentration, colligative properties, and solubility rules
O) exemplify basic acid/ base chemistry principles
P) calculate the energy relationships that occur during physical and chemical changes
Grading Policies
Grade Scale- Grades are calculated out of a total-running-point system
*The teacher reserves the right to make announced adjustments to the point system.
Unit Grades
Tests- 50 pts
Projects- 50 pts
Lab Reports- 25 pts
Quizzes- 10-20 pts
Problem Sets- 15 pts
Other Homework- 5pts
Quarter Grades
Journal- 20
Portfolio- 20
Participation- 20
Late Work Expectations
- To earn full credit on assignments, work must be completed and turned in at the beginning of the period on the day it is due.
- Graded homework will be accepted the next day for half credit.
- Major projects/reports turned in beyond the initial due date drop a full letter grade each class
day until it becomes an “F”.
Make Up Work
- Students are expected to make arrangements regarding absent work in advance.
- The student is responsible for checking their class assignment binder, for copies of handouts and assignment details on the day of his/her return to be prepared for the next class.
The student is responsible for seeing his/her teacher OUTSIDE of class time to inquire about
make up/absent work.
Plagiarism/Integrity: See student handbook.
Behavior Expectations & Classroom Conduct
NOTE: The chemistry classroom and lab area are unique places and special requirements for dress and conduct are mandated by the State of Maine. During lab activities no food or drink is permitted, appropriate personal protection equipment must be worn, and all general safety rules must be complied with. See Lab Safety Rules: Student Contract for additional details.
Be polite and respectful to everyone else and to yourself. No foul language.
Be prompt, on time for class & quick with breaks.
Be prepared for class. (This means that you need your journal, writing utensil, calculator, completed assignments, and your focused mind.)
Be productive, stay on task from the beginning to the end of class. Participation is graded.
Be positive, make the best of situations and opportunities.
Personal Electronic Devices are not allowed during class and will be reported/ confiscated according to the school’s policy.
Behavior that falls outside the contracted rules will be dealt with swiftly and justly at the teacher’s discretion.
Course Schedule
Order and timeline of units described below may vary according to student response to the material.
Topic
Students Will Be Able To
Assessment(s) (Quizzes/Labs/Exams)
Time
MLR
Unit 1 Matter
-Distinguish between the chemical and physical properties of matter.
-Use the proper units when making measurements and calculations.
- Identify elements, mixtures and compounds.
Test, Quizzes L- Measuring density of solids and liquids.
L- Chemical change vs Physical change
4-6
A2 a C1 a, c, e D3 a
Unit 2 Atoms Molecules and Ions
-Explain the development of the modern atomic theory.
-Use the periodic table to determine the structure of an atom.
-Calculate the average atomic mass of an element from the relative abundance of its isotopes.
-Identify names and symbols of common elements.
Tests, Quizzes
L- Candy Atoms
L- Bean Bag Isotopes
5-7
A2 a C1 a, c, e D3 a, b
Unit 3 Periodic Relationships
- Explain the composition of the Periodic Table.
-Describe periodic variation of properties: Ionization Energy, Atomic Radii, Electronegativity
Tests, Quizzes
L- Reactivity Lab
Plotting Trends
4-6
A1 a, b A3 a B1 a D3 a, b
Unit 4 Electronic Structure of the Atom
-Use Quantum numbers, Atomic Orbitals, Electron Configuration Rules, and the Aufbau Principle to identify elements.
Tests, Quizzes,
L- Quantum leap.
L- Flame Test
4-6
A4 a C4 a D3 a, b
Unit 5 Chemical Bonding
Topics covered include: Lewis Dot Symbols
Electronegativity
Lewis Structures
Resonance
The Octet Rule
compare the different types of bonds
explain how bonding occurs
Take Home Test, Quizzes
L-Molecular geometry
L-Properties of solids
6-8
A2 a A3 a D3 a, b D4 a, b
Unit 6 Chemical Reactions
- Identify the reactants and products in a chemical reaction and how they follow the law of conservation of mass.
- Identify the five general types of chemical reactions.
- Predict which metals will replace other metals in a compound.
Test, Quizzes L- Identifying Reactions.
L- Activity Series
4-6
B1 a, b C1 a, b, c D3a
Units 7 The Mole and Stoichiometry
-Calculate the relationship between mass, particles, and the mole.
-Convert grams to moles/ moles to grams.
-Use the mole concept to determine mass/moles in a reaction.
Quizzes
LP- Decomposition of Sodium Bicarbonate
6-8
A2 a C1 a, c, e D3 a
Unit 8 Thermo-chemistry
Topics include: Specific Heat Capacity -energy
Energy Changes
Enthalpy
Calorimetry
Colligative properties
Tests, Quizzes,
Lab Heat of fusion of ice Heat capacity of a metal Ice Cream Freezing point
4-6
B1 a, b C4 a D3 a, b
Unit 9 Gases
Topics include: Properties of Gases
Pressure
The Gas Laws
The Ideal Gas Equation
Kinetic Molecular Theory
Tests, Quizzes, L-Boyles Law L-Charles Law Molar mass of a gas
5-7
B1 a, b C1 a, b, c D3 a,
Unit 10 Acids and Bases
Identify properties and calculate the products of acid/base reactions.
Faculty Name: Lora Cyr
Contact: Phone: 207-363-3621 ex182
Email: __lcyr@yorkschools.org__
Room:B-208
Website: School: http://__www.yorkschools.org/yhs__
Class: http://cyrchemclass.wikispaces.com
Welcome Message
College Preparatory Chemistry is a practical approach to the study of chemistry intended to improve students’ chemical literacy and ability to apply new concepts to problem solving situations. The goals of this course are for each student to have a positive science experience in an educationally challenging program and to insure “real world” and college science readiness. Feel free to contact me at any time with questions or concerns. Help is always accessible with appropriate communication.Course Description
Students will explore the mechanisms of matter and chemical reactions through quantitative and qualitative analysis, while developing problem-solving skills, and learning accurate laboratory techniques. The course stresses an understanding of the basic theoretical concepts of chemistry with a strong emphasis on measurement and calculation. Topics include the atomic and molecular structure, periodicity, chemical bonding, the mole concept, chemical equations and reactions, stoichiometry, gas laws, acid/base reactions, and thermochemistry. Testing and assessment is built on a series of levels from basic knowledge to application and higher order thinking, and several laboratory activities per unit will be used to enhance the understanding of each chemical concept.Required Materials
How to Succeed in this Course:
(1) Attend EVERY class, come prepared and pay attention
(2) Work hard (there are no short-cuts in science)
(3) Think (an often underrated and underemployed skill)
Essential Learning Outcomes
Students will master the following standards through in-class lecture, homework, and lab work. Units are divided into related topics, where order and pace may vary according to student response to the material.
After completing CP Chemistry students will be able to:
Grading Policies
Grade Scale- Grades are calculated out of a total-running-point system
*The teacher reserves the right to make announced adjustments to the point system.
Unit Grades
- Tests- 50 pts
- Projects- 50 pts
- Lab Reports- 25 pts
- Quizzes- 10-20 pts
- Problem Sets- 15 pts
- Other Homework- 5pts
Quarter GradesLate Work Expectations
- To earn full credit on assignments, work must be completed and turned in at the beginning of the period on the day it is due.
day until it becomes an “F”.
Make Up Work
- Students are expected to make arrangements regarding absent work in advance.
- The student is responsible for checking their class assignment binder, for copies of handouts and assignment details on the day of his/her return to be prepared for the next class.
make up/absent work.
Plagiarism/Integrity: See student handbook.
Behavior Expectations & Classroom Conduct
NOTE: The chemistry classroom and lab area are unique places and special requirements for dress and conduct are mandated by the State of Maine. During lab activities no food or drink is permitted, appropriate personal protection equipment must be worn, and all general safety rules must be complied with. See Lab Safety Rules: Student Contract for additional details.
Course Schedule
Order and timeline of units described below may vary according to student response to the material.
(Quizzes/Labs/Exams)
Matter
-Use the proper units when making measurements and calculations.
- Identify elements, mixtures and compounds.
L- Measuring density of solids and liquids.
L- Chemical change vs
Physical change
C1 a, c, e
D3 a
Atoms Molecules and
Ions
-Use the periodic table to determine the structure of an atom.
-Calculate the average atomic mass of an element from the relative abundance of its isotopes.
-Identify names and symbols of common elements.
L- Candy Atoms
L- Bean Bag Isotopes
C1 a, c, e
D3 a, b
Periodic Relationships
-Describe periodic variation of properties: Ionization Energy, Atomic Radii, Electronegativity
L- Reactivity Lab
Plotting Trends
A3 a
B1 a
D3 a, b
Electronic Structure of the Atom
L- Quantum leap.
L- Flame Test
C4 a
D3 a, b
Chemical Bonding
Electronegativity
Lewis Structures
Resonance
The Octet Rule
L-Molecular geometry
L-Properties of solids
A3 a
D3 a, b
D4 a, b
Chemical Reactions
- Identify the five general types of chemical reactions.
- Predict which metals will replace other metals in a compound.
L- Identifying Reactions.
L- Activity Series
C1 a, b, c
D3a
The Mole and Stoichiometry
-Convert grams to moles/ moles to grams.
-Use the mole concept to determine mass/moles in a reaction.
LP- Decomposition of Sodium Bicarbonate
C1 a, c, e
D3 a
Thermo-chemistry
Energy Changes
Enthalpy
Calorimetry
Colligative properties
Lab
Heat of fusion of ice
Heat capacity of a metal
Ice Cream Freezing point
C4 a
D3 a, b
Gases
Pressure
The Gas Laws
The Ideal Gas Equation
Kinetic Molecular Theory
L-Boyles Law
L-Charles Law
Molar mass of a gas
C1 a, b, c
D3 a,
Acids and Bases
L- Antacid Lab
C1 a, b,
D3 b